Question

Aluminum metal has a specific heat of 0.900 j/g•°c. calculate the amount of heat required to raise the temperature of 10.5 moles of al from 30.5 °c to 225°c. a) 1.84 kj
b. 2.41 kj
c. 65.1 kj
d. 49.6 kj
e. 57.3 kj

Answer 1

d.
Q= m·ΔT·C(specific heat)= n·M·ΔT·C=10,5mol·27 g/mol· 194,5(225-30,5)·0,9=49600J=49,6kJ.

Answer 2

The amount of heat required will be "49.6 KJ".

Given:

Mole,

• m = 10.5 moles

Specific heat,

• C = 0.900 j/g•°C

Temperature,

• T = 30.5°C - 225°C

As we know,

→ $Q = m \Delta T C$

By substituting the values, we get

→     $= 10.5\times 27\times 0.9\times (225-30.5)$

→     $=255.15\times (194.5)$

→     $= 49.6 \ KJ$

Thus response above is correct.  

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